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Question

(D) The balanced chemical equation for the reaction of potassium dichromate $(K_2Cr_2O_7)$ with ferrous sulphate $(FeSO_4)$ in an acidic medium is giv

Vedclass · Accepted Answer

$6$

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(D) The balanced chemical equation for the reaction of potassium dichromate $(K_2Cr_2O_7)$ with ferrous sulphate $(FeSO_4)$ in an acidic medium is given by: $Cr_2O_7^{2-} + 14H^+ + 6Fe^{2+} ightarrow 2Cr^{3+} + 6Fe^{3+} + 7H_2O$ From the stoichiometry of the reaction,$1 	ext{ mole}$ of $K_2Cr_2O_7$ reacts with $6 	ext{ moles}$ of $Fe^{2+}$ ions. Therefore,$1 	ext{ mole}$ of potassium dichromate oxidises $6 	ext{ moles}$ of ferrous sulphate.

One mole of potassium dichromate completely oxidises the following number of moles of ferrous sulphate in acidic medium.

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